Inorg. Chem. 1996, 35, 1185
1185
A Proposal for Positive Cooperativity in Anion-Cation Binding in Yttrium and Lutetium Complexes Based on o-Amino-Substituted Phenolate Ligands. On the Way to Coordination Polymers by Self-Assembly. Molecular Structures of [ClLu(OAr)3Na] (X-ray) and [ClY(OAr′)3Y(OAr′)3Na] (X-ray and 89Y-NMR) Marinus P. Hogerheide,† Ste´ phanie N. Ringelberg,† David M. Grove,† Johann T. B. H. Jastrzebski,† Jaap Boersma,† Wilberth J. J. Smeets,‡ Anthony L. Spek,*,‡,§ and Gerard van Koten*,† Department of Metal-Mediated Synthesis, Debye Institute, and Laboratory of Crystal and Structural Chemistry, Bijvoet Center for Biomolecular Research, Utrecht University, Padualaan 8, 3584 CH Utrecht, The Netherlands ReceiVed May 22, 1995X
Unique hetero(poly)metallic complexes [ClM(OAr)3Na] (M ) Lu (3a), Y (3b)) and [ClY(OAr′)3Y(OAr′)3Na] (4) containing the bis (OAr ) OC6H2(CH2NMe2)2-2,6-Me-4) and mono (OAr′ ) OC6H4(CH2NMe2)-2) o-aminosubstituted phenolate ligands have been synthesized and characterized by NMR (1H, 13C, and 89Y) and X-ray structure determinations (3a and 4). Crystals of 3a are triclinic, space group P1h, with unit cell dimensions a ) 10.706(1) Å, b ) 14.099(2) Å, c ) 18.882(3) Å, R ) 93.48(1)°, β ) 99.49(1)°, γ ) 108.72(11)°, and Z ) 2. The chlorine, lutetium, and sodium atoms in 3a lie on a pseudo-3-fold axis (∠Cl-Lu‚‚‚Na ) 177.82(5)°) around which the three phenolate ligands are arranged in such a way that a “propeller-like” molecule with screw-type chirality results. Crystals of 4 are triclinic, space group P1, with unit cell dimensions a ) 11.411(4) Å, b ) 13.325(4) Å, c ) 13.599(4) Å, R ) 88.91(3)°, β ) 65.44(2)°, γ ) 72.77(3)°, and Z ) 1. In 4 the chlorine, the two yttrium and the sodium atoms lie on a pseudo-3-fold axis (Cl-Y(1)‚‚‚Y(2)‚‚‚Na: ∠Cl-Y‚‚‚Y ) 179.36(8)° and ∠Y‚‚‚Y‚‚‚Na ) 178.38(10)°) around which the six phenolate ligands are arranged in two shells of three ligands. One shell bridges the yttrium atoms in an asymmetric fashion, while the second shell bridges the second yttrium and the sodium atom, resulting in two shells of opposite screw-type chirality. 1H, 13C, and 89Y (for 3b and 4) NMR confirmed that the structures found for 3a and 4 in the solid state are retained in solution. For 4 89Y NMR showed two separate resonances (202.4 and 132.4 ppm), with 2JYY ) 0.4 Hz. The formation of 3a and 3b is described as resulting from positive cooperativity in anion-cation bonding: coordination of chloride anion to a neutral metal tris(phenolate) leads to preorganization of available binding sites in the resulting anionic complex for the binding of the sodium cation. In 4 this cooperativity is the driving force for the self-assembly of an anionic bimetallic molecular structure with available, preorganized binding sites for the capture of the cation. A proposal is made to use these observations for the possible synthesis of new coordination polymers.
Introduction Lanthanide and group 3 alkoxide complexes that are volatile and/or soluble in organic solvents have a great potential as precursors for the preparation of lanthanide containing oxide materials by either the MOCVD1 or the sol-gel technique.2 The * To whom correspondence should be addressed. † Debye Institute, Utrecht University. ‡ Bijvoet Center for Biomolecular Research. § Address correspondence regarding the crystallography to this author. X Abstract published in AdVance ACS Abstracts, January 1, 1996. (1) (a) Desu, S. B., Beach, D. B., Wessels, B. W., Gokoglu, S., Eds. MetalOrganic Chemical Vapor Deposition of Electronic Ceramics. Mater. Res. Soc. Symp. Proc. 1994, 335. (b) Bradley, D. C. Chem. ReV. 1989, 89, 1317. (c) Hubert-Pfalzgraf, L. G.; Massiani, M. C.; Papiernik, R.; Poncelet, O. J. Phys. Colloq. 1989, 50, C5-981. (d) Deacon, G. B.; MacKinnon, P.; Dickson, R. S.; Pain, G. N.; West, B. O. Appl. Organomet. Chem. 1990, 4, 439. (2) (a) Brinker, C. J., Clark, D. E., Ulrich, D. R., Eds. Better Ceramics Through Chemistry II. Mater. Res. Soc. Symp. Proc. 1986, 73. (b) Hubert-Pfalzgraf, L. G. New J. Chem. 1987, 11, 663. (c) Transformation of Organometallics into Common and Exotic Materials; Laine, R. M., Ed.; Martinus Nijhoff: Dordrecht, 1988; pp 207-235 (Ulrich, D. R.) and pp 261-278 (Rinker, C. J.). (d) Hirano, S.; Hayashi, T.; Miura, M.; Tomanaga, H. Bull. Chem. Soc. Jpn. 1989, 62, 888. (e) Goel, S. C.; Kramer, K. S.; Gibbons, P. C.; Buhro, W. E. Inorg. Chem. 1989, 28, 3619. (f) Sanchez, C.; Livage, J. New J. Chem. 1990, 14, 513. (g) Sauer, N. N.; Garcia, E.; Salazar, K. V.; Ryan, R. R.; Martin, J. A. J. Am. Chem. Soc. 1990, 112, 1524.
0020-1669/96/1335-1185$12.00/0
use of a precursor in which different metal ions are incorporated in the appropriate ratio is known to increase the quality of the resulting (semiconductor) material3 and as a consequence heterometallic alkoxides4 and a number of preceramic mixedmetal alkoxide aggregates5 have been prepared. In addition, lanthanide alkoxides have been found to be active catalysts in a variety of processes.6,7 Although lanthanide and group 3 metal alkoxides and aryloxides typically are polymeric, hydrocarbon (3) Cowley, A. H.; Jones, R. A. Angew. Chem., Int. Ed. Engl. 1989, 28, 1208. (4) For a review on heterometallic alkoxides, see: Caulton, K. G.; HubertPfalzgraf, L. G. Chem. ReV. 1990, 90, 969. (5) (a) Blake, A. J.; Milne, P. E. Y.; Thornton, P.; Winpenny, R. E. P. Angew. Chem., Int. Ed. Engl. 1991, 30, 1139. (b) Wang, S. Inorg. Chem. 1991, 30, 2252. (c) Coan, P. S.; Huffman, J. C.; Caulton, K. G. Inorg. Chem. 1992, 31, 4207. (d) Miele, P.; Foulon, J. D.; Hovnanian, N.; Cot, L. J. Chem. Soc., Chem. Commun. 1993, 29. (e) Bidell, W.; Do¨ring, J.; Bosch, H. W.; Hund, H.-U.; Plappert, E.; Berke, H. Inorg. Chem. 1993, 32, 502. (f) Labrize, F.; Hubert-Pfalzgraf, L. G.; Daran, J.-C.; Halut, S. J. Chem. Soc., Chem. Commun. 1993, 1556. (g) Wang, S.; Pang, Z.; Smith, K. D. L.; Wagner, M. J. J. Chem. Soc., Dalton Trans. 1994, 955. (6) (a) Namy, J. L.; Souppe, J.; Collin, J.; Kagan, H. B. J. Org. Chem. 1984, 49, 2045. (b) Lebrun, A.; Namy, J. L.; Kagan, H. B. Tetrahedron Lett. 1991, 32, 2355. (c) Sasai, H.; Suzuki, T.; Arai, S.; Arai, T.; Shibasaki, M. J. Am. Chem. Soc. 1992, 114, 4418. (d) Ohno, H.; Mori, A.; Inoue, S. Chem. Lett. 1993, 375. (e) Sasai, H.; Suzuki, T.; Itoh, N.; Shibasaki, M. Tetrahedron Lett. 1993, 34, 851.
© 1996 American Chemical Society
1186 Inorganic Chemistry, Vol. 35, No. 5, 1996
Hogerheide et al. also bind in the zwitterionic form, i.e. as an ammonium phenolate, binding Via O- to the metal and forming additional hydrogen bridges through the -(NR1R2)H group.21 In the course of this work we observed some unique examples of cooperative anion-cation bonding, which appeared as the driving force for self-assembly of heteropolymetallic complexes.19 This is exemplified by the synthesis and structural features of some hetero(poly)metallic complexes derived from bis(ortho)-chelating HOC6H2(CH2NMe2)2-2,6-Me-4 and mono(ortho)-chelating HOC6H4(CH2NMe2)-2. These complexes potentially show the way to a new type of organometallic polymeric materials and might be used as precursors for preceramic mixed-metal complexes. Experimental Section
Figure 1. o-Aminophenolate ligands and their coordination possibilities: monodentate (a, b),20 bidentate (c, d),15,16,20 and bridging between identical (M ) M′)17,18 or different (M * M′)19 metal centers (e).
insoluble materials,8,9 solvent-free complexes are known of sterically demanding ligands (i.e. OCMeEtiPr,10 OC6H2tBu2-2,6Me-411 ), or of ligands containing potentially intramolecularly coordinating substituents (i.e. OCtBu2CH2PMe2,12 OC6H3Ph22,6 13 ).14 Recently, we have become interested in group 3 and lanthanide metal complexes with available Lewis acidic sites that might be used to activate aromatic halides toward nucleophilic substitution. To this end we have applied o-amino substituted phenolate ligands of the type HOC6H2(CH2N(R1)R2)-2-X-6-R-4 (X ) H, CH2NR1R2) which in their respective phenolate complexes display a variety of coordination geometries15-20 (see Figure 1). Moreover, recently we established that neutral phenols can (7) (a) Schumann, H.; Muller, J.; Genthe, W. Abstract of papers; IX International Conference on Organometallic Chemistry, Dijon, France, 1979; Abstract C60. (b) Schumann, H.; Genthe, W.; Bruncks, N.; Pickardt, J. Organometallics 1982, 1, 1194. (c) Evans, W. J.; Hanusa, T. P.; Levan K. R. Inorg. Chim. Acta 1985, 110, 191. (d) Lappert, M. F.; Smith, R. G. Presented at The Second International Conference on the Basic and Applied Chemistry of f-Transition and Related Elements, Lissabon, 1987; Abstract P(II)1. (e) Hitchcock, P. B.; Lappert, M. F.; Smith, R. G.; Bartlett, R. A.; Power, P. P. J. Chem. Soc., Chem. Commun. 1988, 1007. (f) Heeres, H. J.; Meetsma, A.; Teuben, J. H. J. Chem. Soc., Chem. Commun. 1988, 962. (8) For a review on lanthanide alkoxide chemistry until 1990 see: Mehrotra, R. C.; Singh, A.; Tripathi, U. M. Chem. ReV. 1991, 91, 1287. (9) Bradley, D. C.; Mehrotra, R. C.; Gaur, D. P. Metal Alkoxides; Academic Press: London, 1978. (10) Bradley, D. C.; Chudzynska, H.; Hursthouse, M. B.; Motevalli, M. Polyhedron 1991, 10, 1049. (11) Hitchcock, P. B.; Lappert, M. F.; Singh, A. J. Chem. Soc., Chem. Commun. 1983, 1499. (12) Hitchcock, P. B.; Lappert, M. F.; MacKinnon, I. A. J. Chem. Soc., Chem. Commun. 1988, 1557. (13) Deacon, G. B.; Nickel, S.; MacKinnon, P.; Tiekink, E. R. T. Aust. J. Chem. 1990, 43, 1245. (14) Herrmann, W. A.; Anwander, R.; Denk, M. Chem. Ber. 1992, 125, 2399. (15) van der Schaaf, P. A.; Jastrzebski, J. T. B. H.; Hogerheide, M. P.; Smeets, W. J. J.; Spek, A. L.; van Koten, G. Inorg. Chem. 1993, 32, 4111. (16) Alsters, P. L.; Teunissen, H. T.; Boersma, J.; Spek, A. L.; van Koten, G. Organometallics 1993, 12, 4691. (17) (a) van der Schaaf, P. A.; Jastrzebski, J. T. B. H.; Hogerheide, M. P.; Smeets, W. J. J.; Spek, A. L.; van Koten, G. Inorg. Chem. 1993, 32, 4111. (b) Hogerheide, M. P.; Ringelberg, S. N.; Janssen, M. D.; Boersma, J.; Spek, A. L.; van Koten, G. Inorg. Chem. 1996, 35, 1195.
General Data. All reactions were performed using standard Schlenk techniques in an atmosphere of dry, oxygen-free dinitrogen. All solvents were carefully dried and distilled prior to use. Anhydrous LuCl3 and YCl3 were purchased from Strem Chemicals Inc. The phenols HOC6H4(CH2NMe2)-2 (1) and HOC6H2(CH2NMe2)2-2,6-Me-4 (2), as well as their sodium salts NaOC6H4(CH2NMe2)-2 and NaOC6H2(CH2NMe2)2-2,6-Me-4 were synthesized according to literature procedures.15 Elemental analyses were performed by Kolbe Mikroanalytisches Laboratorium, Mu¨lheim, Germany. 1H and 13C NMR data were collected on Bruker AC200 and AC300 instruments. EI-MS spectra (70 eV) were recorded using the direct inlet probe of a Unicam Automass GC-MS spectrometer. 89Y NMR Spectroscopy. 89Y NMR spectra were recorded on a Bruker AC200 spectrometer at a transmitter frequency of 9.807 MHz, using 10 mm tubes. Concentrations were 0.6 M (3b) and 1.5 M (4) in C6D6 and CDCl3, respectively. Because of the long relaxation times of 89Y, a delay of 60 s was used at a pulse width of 20 µs. A satisfactory signal to noise ratio was typically obtained by accumulation of 40 transients with 16K data acquisition points and a spectral width of 3 kHz. To ensure that the observed chemical shifts did not arise from foldovers, the transmitter offset was varied. The chemical shifts are referenced to 3 M YCl3 in D2O (0.0 ppm). {ClLu[OC6H2(CH2NMe2)2-2,6-Me-4]3Na} (3a). To a stirred suspension of LuCl3 (2.11 g; 7.50 mmol) in THF (50 mL) a solution of NaOC6H2(CH2NMe2)2-2,6-Me-4 (5.50 g; 22.5 mmol) in THF (100 mL) was added dropwise at room temperature. After the mixture was stirred overnight at room temperature, the solvent was removed in Vacuo. The resulting residue was extracted twice with hexane (80 mL). Evaporation of the combined hexane fractions gave the product 3a as a yellow, crystalline solid (5.38 g; 80%). Mp: 180 °C dec. Yellow crystals suitable for an X-ray structure determination were grown by allowing a concentrated toluene solution to cool to room temperature. 1H NMR data for 3a (C D , 200 MHz, 298 K): δ 6.81 (s, 6 H, Ar), 6 6 4.42 (br, 3 H, CH(H)N), 3.79 (br, 3 H, CH(H)N), 3.29 (br, 3 H, CH(H)N), 2,84 (br, 3 H, CH(H)N), 2.45 (s, 18 H, N(Me)2), 2.26 (s, 9 H, p-Me), 1.74 (s, 18 H, NMe2). 13C NMR data for 3a (C6D6, 50 MHz, 298 K): δ 161.72 (CO), 132.64, 131.62, 125.80, 122.50 (Ar), 65.81 (CH2N), 63.01 (CH2N), 47.03 (NMe2), 46.19 (NMe2), 20.65 (p-Me). Anal. Calcd for C39H63N6O3LuNaCl‚1.5C7H8: C, 57.41; H, 7.30; N, 8.12. Found: C, 56.97; H, 6.79; N, 8.18. {ClY[OC6H2(CH2NMe2)2-2,6-Me-4]3Na} (3b). The preparation of 3b was identical to that of 3a. Addition of a solution of NaOC6H2(CH2NMe2)2-2,6-Me-4 (5.50 g; 22.5 mmol) in THF (100 mL) to a stirred (18) (a) van der Schaaf, P. A.; Hogerheide, M. P.; Grove, M. D.; Spek, A. L.; van Koten, G. J. Chem. Soc., Chem. Commun. 1992, 1703. (b) Tesh, K. F.; Hanusa, T. P. J. Chem. Soc., Chem. Commun. 1991, 879. (c) Gultneh, Y.; Farooq, A.; Liu, S.; Karlin, K. D.; Zubieta, J. Inorg. Chem. 1992, 31, 3607. (d) Teipel, S.; Griesar, K.; Haase, W.; Krebs, B. Inorg. Chem. 1994, 33, 456. (19) Hogerheide, M. P.; Jastrzebski, J. T. B. H.; Boersma, J.; Smeets, W. J. J.; Spek, A. L.; van Koten, G. Inorg. Chem. 1994, 33, 4431. (20) Hogerheide, M. P.; Wesseling, M.; Jastrzebski, J. T. B. H.; Boersma, J.; Kooijman, H.; Spek, A. L.; van Koten, G. Organometallics 1995, 14, 4483. (21) Hogerheide, M. P.; Ringelberg, S. N.; Jastrzebski, J. T. B. H.; Boersma, J.; Spek, A. L.; van Koten, G. To be submitted for publication.
Binding in Yttrium and Lutetium Complexes suspension of YCl3 (1.46 g; 7.50 mmol) and subsequent workup afforded 3b as a yellow, crystalline solid (4.87 g; 80%). Mp: 170 °C dec. 1H NMR data for 3b (C D , 200 MHz, 298 K): δ 6.79 (s, 6 H, Ar), 6 6 2.48 (s, 18 H, NMe2), 2.25 (s, 9 H, p-Me), 1.70 (s, 18 H, NMe2). 1H NMR data for 3b (C6D6, 200 MHz, 263 K): δ 6.77 (s, 3 H, Ar), 6.75 (s, 3 H, Ar), 5.19 (d, 3 H, 2JHAHB ) 12 Hz, CHAHBN), 4.21 (d, 3 H, 2J HCHD ) 10 Hz, CHCHDN), 2.65 (d, 3 H, JHBHA ) 12 Hz, CHAHBN), 2.51 (s, 18 H, NMe2), 2.27 (s, 9H, p-Me), 2.16 (d, 3 H, 2JHDHC ) 10 Hz, CHCHDN), 1.55 (s, 18 H, NMe2). 1H NMR data for 3b (C6D6, 200 MHz, 228 K): δ 6.77 (s, 3 H, Ar), 6.76 (s, 3 H, Ar), 5.23 (d, 3 H, 2 JHAHB ) 12 Hz, CHAHBN), 4.25 (d, 3 H, 2JHCHD ) 11 Hz, CHCHDN), 2.63 (d, 3 H, JHBHA ) 12 Hz, CHAHBN), 2.53 (s, 18 H, NMe2), 2.32 (s, 9H, p-Me), 2.16 (d, 3 H, 2JHDHC ) 11 Hz, CHCHDN), 1.63 (s, 9 H, NMeMe), 1.43 (s, 9 H, NMeMe). 13C NMR data for 3b (C6D6, 50 MHz, 298 K): δ 161.79 (CO, 2JYC ) 2.2 Hz), 132.61, 131.72, 125.70, 125.40, 122.26 (Ar), 66.23 (CH2N), 63.24 (CH2N), 46.21 (NMe2), 20.62 (p-Me). 13C NMR data for 3b (C6D6, 50 MHz, 228 K): δ 162.12 (CO, 2 JYC ) 2.2 Hz), 133.01, 131.88, 125.63, 125.54, 122.11 (Ar), 66.86 (CH2N), 63.22 (CH2N), 48.37 (NMe2), 45.05 (NMe2), 44.82 (NMe2), 20.99 (p-Me). MS (EI), m/z (%): 776 (0.39) [M+ - Cl]. 89Y NMR data for 3b (CDCl3, 9.804 MHz, 298 K): δ 160.9. Anal. Calcd for C39H63N6O3YNaCl: C, 57.74; H, 7.83; N, 10.36. Found: C, 57.79; H, 7.96; N, 10.30. [ClY{µ-OC6H4(CH2NMe2)-2}3Y{OC6H4(CH2NMe2)-2}3Na] (4). To a stirred suspension of YCl3 (1.46 g; 7.50 mmol) in THF (25 mL) a solution of NaOC6H4(CH2NMe2)-2 (3.90 g; 22.5 mmol) in THF (50 mL) was added dropwise at room temperature. After the mixture was stirred overnight, the solvent was removed in Vacuo. The residue was extracted twice with CH2Cl2 (80 mL). Removal of the solvent in Vacuo and subsequent washing of the resulting residue with pentane (40 mL) gave the product as a white solid in quantitative yield (8.53 g). Mp > 200 °C. Colorless hexagonal crystals of 4, suitable for an X-ray analysis, were grown by allowing a hot benzene solution to cool to room temperature. 1H NMR data for 4 (C D , 300 MHz, 298 K): δ 7.18 (m, 1 H, Ar), 6 6 7.05 (m, 2 H, Ar), 6.87 (m, 1 H, Ar), 6.75 (m, 1 H, Ar), 6.61 (d, 1 H, Ar), 6.51 (d, 1H, Ar), 5.80 (d, 1 H, Ar), 4.95 (d, 1 H, 2JHAHB ) 12 Hz, CHAHBN), 4.37 (d, 1 H, 2JHCHD ) 11 Hz, CHCHDN), 2.43 (d, 1 H, 2J 2 HBHA ) 12 Hz, CHBHAN), 2.26 (d, 1 H, JHDHC ) 11 Hz, CHDHCN), 1.99 (s, 3 H, NMeMe), 1.94 (s, 3 H, NMeMe), 1.62 (s, 6 H, NMe2). 1H NMR data for 4 (CDCl3, 300 MHz, 298 K): δ 7.18 (d, 1 H, Ar), 7.03 (t, 1 H, Ar), 6.88 (m, 3 H, Ar), 6.50 (t, 1 H, Ar), 6.29 (d, 1 H, Ar), 5.32 (d, 1 H, Ar), 4.90 (d, 1 H, 2JHAHB ) 12 Hz, CHAHBN), 4.03 (d, 1 H, 2JHCHD ) 11 Hz, CHCHDN), 2.75 (d, 1 H, 2JHBHA ) 12 Hz, CHBHAN), 2.37 (s, 3 H, NMeMe), 2.30 (s, 3 H, NMeMe), 2.12 (d, 1 H, 2JHDHC ) 11 Hz, CHDHCN), 1.66 (s, 6 H, NMe2). 13C NMR data for 4 (CDCl3, 75 MHz, 298 K): δ 164.24 (d, 2JYC ) 4.0 Hz, CO), 160.01 (d, 2JYC ) 0.6 Hz, CO), 132.22-114.53 (Ar), 64.71 (CH2N), 61.79 (CH2N), 46.57, 46.37, 45.90 (NMe2). 89Y NMR data for 4 (CDCl3, 9.804 MHz, 298 K): δ 202.4 (d, 2JYY ) 0.4 Hz), 132.4 (d, 2JYY ) 0.4 Hz). Anal. Calcd for C54H72ClN6NaO6Y2: C, 57.02; H, 6.38; N, 7.32. Found: C, 57.07; H, 6.49; N, 7.32. X-ray Data Collection and Structure Refinement. A yellow, block-shaped crystal of 3a and a colorless crystal of 4 were each sampled from below the liquid surface directly into a viscous oil to avoid loss of crystallinity (Vide infra), glued on top of a glass fiber, and transferred into the cold nitrogen stream on an Enraf-Nonius CAD4T rotating anode diffractometer, using graphite-monochromated Mo KR radiation, for data collection. Accurate unit-cell parameters were determined by least-squares treatment of 25 well-centered reflections (SET4) in the range 11.4 < θ < 14.7° and 9.8 < θ < 13.6° for 3a and 4, respectively. All data were collected in ω/2θ scan mode. Crystal data and details on data collection and refinement are collected in Table 1. Final coordinates for the non-hydrogen atoms are given in Tables 2 and 3, selected bond distances and angles in Tables 4 and 5 for 3a and 4, respectively. Data were corrected for Lp effects and for the observed linear decay of the reference reflections. Data for 4 were also corrected for absorption (DIFABS;22 correction range 0.827(22) Walker, N.; Stuart, D. Acta Crystallogr., Sect. A 1983, 39, 158.
Inorganic Chemistry, Vol. 35, No. 5, 1996 1187 Table 1. Crystallographic Data for 3a and 4 formula fw space group a, Å b, Å c, Å R, deg β, deg γ, deg V, Å3 Fcalc, g cm-3 Z µ, cm-1 T, K radiation; λ, Å final R b final wR2c final Rwd
3a
4
C39H63N6O3NaLuCl‚ 1.5C7H8 1035.58a P1h (No. 2) 10.706(1) 14.099(2) 18.882(3) 93.48(1) 99.49(1) 108.72(11) 2642.7(6) 1.301a 2 20.7a 300 Mo KR; 0.71073 0.0411
C54H66N6O6NaY2Cl‚ 2.69C6H6 1339.73a P h 1 (No. 1) 11.411(4) 13.325(4) 13.599(4) 88.91(3) 65.44(2) 72.77(3) 1783.3(11) 1.248a 1 17.2a 150 Mo KR; 0.71073 0.062 [6352 Fo > 4σ(Fo)] 0.1453
0.0454
2.69 benzene solvate molecules included. b R ) ∑||Fo| - |Fc||/ ∑|Fo|. c wR2 ) [∑[w(Fo2 - Fc2)2]/∑[w(Fo2)2]]1/2. d Rw ) [∑[w(||Fo| |Fc||)2/∑[w(Fo2)]]1/2. a
1.133). The structures were solved by Patterson (3a: DIRDIF)23 or direct methods (4: SIR92)24 and subsequent difference Fourier techniques. Refinement was carried out by full-matrix least-squares techniques on F (3a: SHELX76)25 or on F2 (4: SHELXL93).26 Hydrogen atoms were introduced on calculated positions and included in the refinement riding on their carrier atoms. All non-hydrogen atoms were refined with anisotropic thermal parameters. The unit cell of 3a contains a cavity of 745 Å3, located around an inversion site, which contains three toluene solvate molecules. Similarly, the unit cell of 4 contains a cavity of 561 Å3, which contains 2.7 benzene solvate molecules. These toluene and benzene molecules could not be located unambiguously from difference Fourier maps and were taken into account in the structure factor and refinement calculations by Fourier transformation of the diffuse electron density in the cavity (Bypass procedure).27 The structure determination for 4 showed some disorder in the position of Y(1), Na and Cl, which was modeled by inverting the positions of these atoms through the position of Y(2). The hydrogen atoms of 3a were refined with a common isotropic atomic displacement parameter: U ) 0.087(3) Å2. The hydrogen atoms of 4 were refined with a fixed isotropic thermal parameter amounting to 1.5 or 1.2 times the value of the equivalent isotropic thermal parameter of their carrier atoms, for the methyl hydrogen atoms and the other hydrogen atoms respectively. Weights were introduced in the last refinement cycles. Neutral atom scattering factors were taken from Cromer and Mann28 and corrected for anomalous dispersion29 for 3a. Neutral atom scattering factors and anomalous dispersion corrections were taken from ref 30 for 4. All calculations were carried out on a DECstation 5000 cluster. Geometrical calculations and ORTEP drawings were done with PLATON.31 All other drawings were made with PLUTON.32 (23) Beurskens, P. T.; Admiraal, G.; Beurskens, G.; Bosman, W. P.; Garcı´aGranda, S.; Gould, R. O.; Smits, J. M. M.; Smykalla, C. The DIRDIF program system. Technical Report of the Crystallography Laboratory, University of Nijmegen, The Netherlands, 1992. (24) Altomare, A.; Cascarano, G.; Giacovazzo, C.; Guagliardi, A. J. Appl. Cryst. 1993, 26, 343. (25) Sheldrick, G. M. SHELX76. Crystal structure analysis package. University of Cambridge, Cambridge, England, 1976. (26) Sheldrick, G. M. SHELXL-93. Program for crystal structure refinement. University of Go¨ttingen, Germany, 1993. (27) van der Sluis, P.; Spek, A. L. Acta Crystallogr., Sect. A 1990, 46, 194. (28) Cromer, D. T.; Mann, J. B. Acta Crystallogr., Sect. A 1968, 24, 321. (29) Cromer, D. T.; Liberman, D. J. Chem. Phys. 1970, 53, 1891. (30) International Tables for Crystallography, Volume C; Wilson, A. J. C., Ed.; Kluwer Academic Publishers: Dordrecht, The Netherlands, 1992. (31) Spek, A. L. Acta Crystallogr., Sect. A 1990, 46, C34. (32) Spek, A. L., PLUTON, molecular graphics program. Utrecht University, Utrecht, The Netherlands, 1995.
1188 Inorganic Chemistry, Vol. 35, No. 5, 1996
Hogerheide et al.
Table 2. Final Coordinates and Equivalent Isotropic Thermal Parameters of the Non-Hydrogen Atoms for 3a atom
x
y
z
Ueq (Å2)a
Lu Cl Na O(1) O(2) O(3) N(1) N(2) N(3) N(4) N(5) N(6) C(1) C(2) C(3) C(4) C(5) C(6) C(7) C(8) C(9) C(10) C(11) C(12) C(13) C(14) C(15) C(16) C(17) C(18) C(19) C(20) C(21) C(22) C(23) C(24) C(25) C(26) C(27) C(28) C(29) C(30) C(31) C(32) C(33) C(34) C(35) C(36) C(37) C(38) C(39)
0.76994(2) 0.51813(13) 1.0793(2) 0.8586(3) 0.9662(3) 0.8774(3) 0.6170(4) 1.1517(5) 1.2756(4) 0.7499(4) 0.7507(4) 1.1144(5) 0.8560(5) 0.7750(5) 0.7737(6) 0.8504(7) 0.9304(6) 0.9366(5) 0.7019(6) 0.5165(6) 0.5462(7) 0.8468(9) 1.0306(6) 1.2268(8) 1.2353(6) 1.0313(5) 1.1490(5) 1.2064(6) 1.1592(7) 1.0515(7) 0.9881(5) 1.2114(5) 1.3899(6) 1.3232(7) 1.2214(9) 0.8829(6) 0.6627(6) 0.6927(6) 0.9249(4) 0.9207(5) 0.9655(6) 1.0190(7) 1.0271(6) 0.9839(5) 0.8810(5) 0.7304(6) 0.6439(5) 1.0673(10) 1.0016(5) 1.1093(8) 1.2416(6)
0.85892(2) 0.85386(12) 0.86261(15) 0.8263(3) 0.9752(2) 0.7736(2) 0.6753(3) 0.9084(4) 1.0052(3) 1.0131(3) 0.8950(3) 0.6855(3) 0.7559(4) 0.6554(4) 0.5856(5) 0.6113(6) 0.7099(5) 0.7836(4) 0.6189(4) 0.6727(6) 0.6211(5) 0.5319(7) 0.8880(4) 1.0186(6) 0.8537(6) 1.0732(4) 1.1246(4) 1.2269(4) 1.2836(5) 1.2309(5) 1.1276(4) 1.0667(4) 1.0694(5) 0.9459(5) 1.3969(5) 1.0716(4) 0.9658(5) 1.0830(5) 0.7569(3) 0.8144(4) 0.7934(5) 0.7161(6) 0.6606(5) 0.6807(4) 0.9074(4) 0.9935(5) 0.8175(5) 0.6915(8) 0.6255(4) 0.6378(5) 0.6936(5)
0.24041(1) 0.23395(8) 0.24173(11) 0.15227(18) 0.27397(17) 0.29896(17) 0.1789(2) 0.1110(3) 0.3409(2) 0.1708(2) 0.3744(2) 0.2763(3) 0.1011(3) 0.0984(3) 0.0427(3) -0.0101(4) -0.0054(3) 0.0489(3) 0.1584(3) 0.1137(3) 0.2324(4) -0.0694(5) 0.0542(3) 0.1195(4) 0.0896(4) 0.2750(3) 0.3274(3) 0.3291(4) 0.2827(4) 0.2274(4) 0.2224(3) 0.3767(3) 0.3152(4) 0.3931(4) 0.2877(5) 0.1568(3) 0.0998(3) 0.2034(4) 0.3645(3) 0.4267(3) 0.4954(3) 0.5043(3) 0.4424(3) 0.3730(3) 0.4221(3) 0.3831(3) 0.3984(3) 0.5797(4) 0.3077(3) 0.2052(3) 0.3223(4)
0.0365(1) 0.0578(5) 0.0506(7) 0.0474(12) 0.0425(11) 0.0427(11) 0.0521(16) 0.0657(19) 0.0520(16) 0.0506(17) 0.0425(14) 0.0559(17) 0.0473(17) 0.0525(17) 0.075(2) 0.089(3) 0.074(3) 0.0500(19) 0.0564(17) 0.078(2) 0.075(3) 0.137(4) 0.0548(19) 0.106(3) 0.087(3) 0.0443(17) 0.0491(17) 0.065(2) 0.075(3) 0.072(3) 0.0499(17) 0.0495(17) 0.074(3) 0.079(3) 0.118(4) 0.058(2) 0.073(3) 0.072(3) 0.0380(16) 0.0436(17) 0.060(2) 0.074(3) 0.063(2) 0.0474(17) 0.0453(17) 0.063(2) 0.0587(19) 0.123(5) 0.0541(19) 0.083(3) 0.068(2)
a
U(eq) ) one-third of the trace of the orthogonalized U.
Results Syntheses and Properties. Reaction of lutetium or yttrium trichloride with 3 equiv of NaOC6H2(CH2NMe2)2-2,6-Me-4 or NaOC6H4(CH2NMe2)-2 at room temperature in THF, resulted in the formation of heterometallic complexes Na[M(OAr)3]xCl (x ) 1, OAr ) OC6H2(CH2NMe2)2-2,6-Me-4, M ) Lu (3a), Y (3b); x ) 2, OAr ) OC6H4(CH2NMe2)-2, M ) Y (4)). These complexes were obtained as crystalline solids in 80% (3a and 3b) or essentially quantitative (4) yield (see Schemes 1 and 2). Complexes 3 and 4 are easily hydrolyzed with formation of the corresponding parent phenols, 2 and 1, respectively. All complexes are soluble in THF and aromatic solvents, while 3a and 3b are also soluble in hexane. The complexes can be (re)crystallized by allowing a hot, concentrated solution in an aromatic solvent to cool to room temperature, with the formation (for all three complexes) of colorless, hexagonal crystals. However, these crystals contain a relatively large
percentage of the crystallization solvent (28 and 31 wt % for 3a and 4, respectively) and lose their crystallinity upon removal of the supernatant liquid, leaving the crystals fragile and nontransparent. Structures in the Solid State. In order to gain insight into the coordination geometries for the metal centers in both the complexes 3 and 4, as well as the incorporation of one NaCl molecule in both these complexes, the solid state structures of 3a and 4 were determined. Complex {ClLu[OC6H2(CH2NMe2)2-2,6-Me-4]3Na}, 3a. The molecular structure (see Figure 2 and Scheme 1) shows 3a to consist of a seven-coordinate lutetium ion surrounded by three phenolate ligands, each bonded through oxygen and coordinating with one of the ortho amino substituents, and one chloride atom. This anionic “ate”-unit still has six available binding sites comprising the remaining three ortho amino substituents and the three phenolate oxygen atoms. These binding sites are arranged in such a way that they form a hexadentate coordination pocket for binding of the sodium cation. The chloride, lutetium, and sodium atoms lie on a pseudo-3-fold axis (∠ClLu‚‚‚Na ) 177.82(5)°), around which the three ligands are arranged (see Figure 3). As a result of the intramolecular coordination of the amino substituents of each bis(amino)phenolate ligand to two different metal centers (Lu and Na), the aromatic ring-plane of each ligand is twisted away from a position perpendicular to the Cl-Lu‚‚‚Na vector, resulting in a “propeller-like” molecule with screw-type chirality. Both enantiomers were present in the measured crystal. As may be expected, the Lu-O bond lengths of 2.143(3) to 2.174(3) Å of the bridging phenolate ligands in 3a are much larger than those of terminal phenolate ligands (e.g. in Lu[OC6H3(iPr)2-2,6]3(THF)2 (5): 2.041(4)-2.048(4) Å).33 The Lu-O-C bond angles in 3a lie in the range 143.0(3) to 145.5(4)°, as a result of their bridging character and the intramolecular coordination of one of the amino substituents to lutetium. Reduction of the M-O-C angle as a result of intramolecular coordination has been observed previously for Yb(OC6H3Ph2-2,6)3, in which the Yb-π-arene interaction of the ytterbium ion with a phenyl substituent of one of the terminal phenolate ligands leads to an even smaller angle of 135.0(3)°.13 The bond angles around the sodium ion show that it is bonded more strongly to one of the phenolate ligands than to the other two. The Na-O(2) bond length of 2.391(4) Å is much shorter than the other Na-O bond lengths (2.550(4) Å and 2.571(4) Å), but is comparable to the Na-O bond lengths in [NaOC6H2(CH2NMe2)2-2,6-Me-4]4 (6).15 In addition, the Na-O(2)-C(14) bond angle of 116.6(3)° differs substantially from the corresponding bond angles found for the other two ligands (105.9(3) and 107.7(3)°). The Na-N bond lengths in 3a fall in a narrow range (2.738(5)-2.759(6) Å), but are much longer than those found in 6 (2.468(3)-2.664(5) Å). So, in the solid state, the sodium ion can be seen as four-coordinate (ON3) with two additional, slightly remote Na-O interactions. An interesting feature concerns the crystal packing of the complex. In this packing the lutetium-chloride vector of one residue points to the sodium ion captured in the pocket of the next residue, thus forming a continuous {(Na‚‚‚Lu-Cl)‚‚‚(Na‚‚‚ Lu-Cl)}n string through the crystal. However, the intermolecular distance between the chloride of one unit and the sodium of the next is at 4.765(3) Å nearly double the sum of the covalent radii (2.53 Å). Complex [ClY{µ-OC6H4(CH2NMe2)-2}3Y{OC6H4(CH2NMe2)-2}3Na], 4. Complex 4 consists of one chlorine atom, two (33) Barnhart, D. M.; Clark, D. L.; Gordon, J. C.; Huffman, J. C.; Vincent, R. L.; Watkin, J. G.; Zwick, B. D. Inorg. Chem. 1994, 33, 3487.
Binding in Yttrium and Lutetium Complexes
Inorganic Chemistry, Vol. 35, No. 5, 1996 1189
Table 3. Final Coordinates and Equivalent Isotropic Thermal Parameters of the Non-Hydrogen Atoms for 4 atom
x
y
z
Ueq (Å2)a
atom
x
y
z
Ueq (Å2)a
Y(1)b Y(2) Clb Nab O(1) O(2) O(3) O(4) O(5) O(6) N(1) N(2) N(3) N(4) N(5) N(6) C(11) C(12) C(13) C(14) C(15) C(16) C(17) C(18) C(19) C(21) C(22) C(23) C(24) C(25) C(26) C(27) C(28) C(29) C(31)
0.03797(13) 0.03070 0.0422(3) 0.0304(4) -0.0741(5) -0.0004(6) 0.1881(6) -0.1455(7) 0.1445(6) 0.0872(6) 0.0780(7) -0.1982(6) 0.2372(7) -0.1594(9) 0.0019(8) 0.2656(8) -0.1336(9) -0.0646(9) -0.1274(10) -0.2565(10) -0.3231(9) -0.2572(11) 0.0710(9) 0.2154(10) -0.0070(11) -0.0795(10) -0.2146(10) -0.2929(11) -0.2464(14) -0.1134(13) -0.0336(11) -0.2770(11) -0.2693(10) -0.2089(11) 0.3284(9)
0.59901(9) 0.85730 0.4026(2) 1.0939(3) 0.7499(4) 0.7266(4) 0.6844(4) 0.9868(4) 0.9179(4) 0.9353(5) 0.5606(5) 0.6230(5) 0.5162(5) 1.2034(6) 1.1545(6) 1.0937(6) 0.7814(7) 0.7324(6) 0.7597(7) 0.8364(8) 0.8863(7) 0.8603(7) 0.6560(7) 0.4892(8) 0.5067(7) 0.7595(7) 0.7561(7) 0.7785(8) 0.8026(9) 0.8143(7) 0.7900(7) 0.7320(8) 0.5975(7) 0.5489(7) 0.6601(7)
0.19023(11) 0.19390 0.1898(2) 0.1997(4) 0.1469(5) 0.3168(5) 0.1073(5) 0.2801(5) 0.2501(5) 0.0542(5) -0.0072(5) 0.3370(5) 0.2406(6) 0.1517(8) 0.3909(6) 0.0453(7) 0.0776(7) -0.0276(7) -0.0985(7) -0.0609(8) 0.0430(8) 0.1065(9) -0.0676(7) -0.0577(8) -0.0257(8) 0.4274(9) 0.4734(8) 0.5748(9) 0.6441(10) 0.6089(9) 0.4943(7) 0.3951(8) 0.2689(8) 0.4152(8) 0.0694(8)
0.0320(4) 0.0346(3) 0.0407(10) 0.0238(12) 0.0471(19) 0.0447(19) 0.048(2) 0.057(2) 0.056(2) 0.052(2) 0.038(2) 0.040(2) 0.042(3) 0.057(3) 0.050(3) 0.056(3) 0.040(3) 0.039(3) 0.054(3) 0.055(4) 0.051(3) 0.049(4) 0.045(3) 0.060(4) 0.067(4) 0.049(4) 0.048(3) 0.067(4) 0.095(5) 0.076(5) 0.041(3) 0.058(4) 0.053(4) 0.059(4) 0.048(3)
C(32) C(33) C(34) C(35) C(36) C(37) C(38) C(39) C(41) C(42) C(43) C(44) C(45) C(46) C(47) C(48) C(49) C(51) C(52) C(53) C(54) C(55) C(56) C(57) C(58) C(59) C(61) C(62) C(63) C(64) C(65) C(66) C(67) C(68) C(69)
0.3965(9) 0.5372(10) 0.6099(10) 0.5434(11) 0.3999(14) 0.3117(9) 0.1640(10) 0.3314(11) -0.2757(10) -0.3289(11) -0.4702(11) -0.5518(13) -0.4827(11) -0.3493(10) -0.2442(11) -0.0874(13) -0.2512(10) 0.2170(9) 0.1624(9) 0.2359(10) 0.3655(10) 0.4223(11) 0.3463(9) 0.0169(9) -0.1411(11) 0.0888(10) 0.1594(12) 0.2862(11) 0.3552(11) 0.3040(14) 0.1772(14) 0.1139(12) 0.3373(8) 0.3292(12) 0.2768(10)
0.6142(6) 0.5807(7) 0.6008(8) 0.6604(8) 0.6941(9) 0.5912(7) 0.4933(8) 0.4145(8) 1.0444(6) 1.1175(7) 1.1672(7) 1.1580(9) 1.0852(8) 1.0327(7) 1.1342(7) 1.2076(10) 1.3036(7) 0.9177(6) 0.9840(6) 0.9760(6) 0.9047(8) 0.8486(7) 0.8558(7) 1.0599(6) 1.2212(7) 1.2160(7) 0.9426(8) 0.9635(8) 0.9585(7) 0.9429(10) 0.9269(9) 0.9246(9) 0.9883(6) 1.1068(9) 1.1748(6)
0.1254(8) 0.0805(10) -0.0188(10) -0.0737(9) -0.0314(11) 0.2416(7) 0.3603(8) 0.1814(10) 0.3344(9) 0.2741(9) 0.3229(10) 0.4264(13) 0.4819(9) 0.4341(9) 0.1586(9) 0.0457(11) 0.2129(9) 0.3063(8) 0.4037(7) 0.4606(7) 0.4223(8) 0.3239(11) 0.2633(7) 0.4449(7) 0.4386(9) 0.3968(8) -0.0520(8) -0.0880(9) -0.2033(8) -0.2717(10) -0.2317(9) -0.1252(11) -0.0167(7) 0.1130(10) -0.0268(7)
0.040(3) 0.060(4) 0.069(4) 0.069(4) 0.082(5) 0.040(3) 0.062(4) 0.075(5) 0.050(4) 0.055(4) 0.066(4) 0.103(6) 0.069(4) 0.051(3) 0.060(4) 0.090(6) 0.063(4) 0.045(3) 0.034(3) 0.051(3) 0.059(4) 0.075(5) 0.042(3) 0.043(3) 0.066(4) 0.053(4) 0.058(4) 0.057(4) 0.059(4) 0.096(6) 0.092(6) 0.081(5) 0.040(3) 0.079(5) 0.051(3)
a
U(eq) ) one-third of the trace of the orthogonalized U. b Disordered atoms (see Experimental Section).
Table 4. Selected Bond Distances and Angles for Complex 3a Lu-Cl Lu-O(1) Lu-O(2) Lu-O(3) Lu-N(1) Lu-N(4) Lu-N(5) C(1)-O(1) C(14)-O(2) Lu-O(1)-C(1) Lu-O(2)-C(14) Lu-O(3)-C(27) Na‚‚‚Lu-Cl
Bond Lengths (Å) 2.6561(15) Na-O(1) 2.143(3) Na-O(2) 2.174(3) Na-O(3) 2.150(3) Na-N(2) 2.649(4) Na-N(3) 2.656(4) Na-N(6) 2.605(4) Lu-Na 1.333(7) C(27)-O(3) 1.330(6) Bond Angles (deg) 145.5(4) Na-O(1)-C(1) 143.0(3) Na-O(2)-C(14) 143.9(3) Na-O(3)-C(27) 177.82(5)
2.550(4) 2.391(4) 2.571(4) 2.759(6) 2.738(4) 2.743(5) 3.292(2) 1.323(6)
105.9(3) 116.6(3) 107.7(3)
yttrium atoms, and one sodium atom lying on a pseudo-3-fold axis (∠Cl-Y(1)-Y(2) ) 179.36(8)°; ∠Y(1)-Y(2)‚‚‚Na ) 178.38(10)°), around which six mono(amino)phenolate ligands are arranged in two separate shells (see Figure 4 and Scheme 2). Three of the phenolate ligands (“first shell”) are associated to both yttrium atoms, each bridging Y(1) and Y(2) with their oxygen atoms and coordinating with their o-amino substituent to Y(1). The distance between the two yttrium atoms is at 3.4189(17) Å only slightly larger than the sum of the covalent radii (3.24 Å).30 The coordination sphere of Y(1) is completed by a chloride atom, making it seven coordinate with a coordination geometry that is fully analogous to that around Lu in 3a. The second group of three phenolate ligands (“second shell”) is bonded through oxygen to Y(2), thus creating a six-coordinate geometry around this Y-center. The three amino substituents of these phenolate ligands form, together with their oxygen
Table 5. Selected Bond Distances and Angles for Complex 4 Y(1)-Cl Y(1)-O(1) Y(1)-O(2) Y(1)-O(3) Y(1)-N(1) Y(1)-N(2) Y(1)-N(3) Y(1)-Y(2) Na-O(4) Na-O(5) Na-O(6) Na-N(4) Na-N(5) Na-N(6) Y(1)-O(1)-C(11) Y(1)-O(2)-C(21) Y(1)-O(3)-C(31) Y(2)-O(1)-C(11) Y(2)-O(2)-C(21) Y(2)-O(3)-C(31) Cl-Y(1)‚‚‚Y(2) Y(1)‚‚‚Y(2)‚‚‚Na
Bond Lengths (Å) 2.603(3) Y(2)-O(1) 2.255(6) Y(2)-O(2) 2.256(6) Y(2)-O(3) 2.236(7) Y(2)-O(4) 2.564(7) Y(2)-O(5) 2.528(7) Y(2)-O(6) 2.576(9) Y(2)-Na 3.4189(17) 2.660(9) O(1)-C(11) 2.557(7) O(2)-C(21) 2.661(8) O(3)-C(31) 2.552(11) O(4)-C(41) 2.596(9) O(5)-C(51) 2.631(11) O(6)-C(61) Bond Angles (deg) 139.0(5) Y(2)-O(4)-C(41) 138.9(6) Y(2)-O(5)-C(51) 135.1(5) Y(2)-O(6)-C(61) 120.1(5) Na-O(4)-C(41) 118.9(5) Na-O(5)-C(51) 122.9(5) Na-O(6)-C(61) 179.36(8) 178.38(10)
2.360(6) 2.391(6) 2.411(6) 2.111(6) 2.096(7) 2.100(6) 3.154(4) 1.369(12) 1.390(13) 1.395(14) 1.333(13) 1.339(13) 1.352(12) 161.1(6) 154.9(5) 155.3(6) 116.3(5) 118.8(5) 117.8(6)
atoms, a six-coordinate pocket for the sodium atom, analogous to the situation observed around Na in 3a. As a result of the coordination of the amino substituents of the first shell of phenolate ligands to Y(1) and of those of the second shell to Na, the aromatic planes of the ligands are tilted from a position perpendicular to the Cl-Y(1)‚‚‚Y(2)‚‚‚Na axis, resulting in two staggered shells of three ligands; these shells have screw-type chiralities with opposite sense (see Figure 4). A view along
1190 Inorganic Chemistry, Vol. 35, No. 5, 1996
Hogerheide et al.
Scheme 1. Synthesis and Schematic Representations of 3a and 3b
Scheme 2. Synthesis and Schematic Representation of 4
the Cl-Y(1)‚‚‚Y(2)‚‚‚Na pseudo-3-fold axis shows this arrangement (see Figure 5). Both the Y-O bond lengths and the Y-O-C bond angles for 4 can be gathered into three groups, as shown in Figure 6. This figure indicates a near-linear relationship between these structural variables. Combination of these structural data for 4 with those of previously reported yttrium phenolate complexes (see Table 6) shows that virtually all the yttrium-phenolate interactions closely follow the trend observed in complex 4 (see Figure 7). The combination of short Y-O bond lengths with large Y-O-C bond angles that are observed for terminal phenolate ligands as well as for the phenolate ligands bridging between Y and Na in 4 (see Figure 7) is relatively common in early-transition metal chemistry and has been explained as resulting from oxygen pπ to metal dπ interactions.34 The only exception to the trend is (C5Me5)Y(OC6H3tBu2-2,6)2 (10),38 which contains one yttrium-phenolate interaction that follows the general trend and one that shows an Y-O-C angle that is “abnormally” acute (128.6(3)°) with respect to the short Y-O bond length of 2.096(4) Å (see Figure 7). The reason for this deviation is not clear. As in complex 3a, one Na-O bond distance in 4 is shorter than the other two: 2.557(7) Å vs 2.660(9) and 2.661(8) Å. These Na-O bond distances are much larger than the corresponding distances in [NaOC6H2(CH2NMe2)2-2,6-Me-4]4 (6),15 (2.325(4)-2.417(2) Å) and indicative of coordinative bonds. The Na-N bond lengths (2.520(17)-2.573(14) Å) are similar to those in 6 and shorter than those in 3a. As in complex 3a (Vide supra), in the crystal packing of 4 the yttrium-chloride vector of one residue points to the sodium ion captured in the pocket of the next, to give parallel “head to tail” cylinders {(Na‚‚‚Y‚‚‚Y-Cl)‚‚‚(Na‚‚‚Y‚‚‚Y-Cl)}n running through the crystal. The intermolecular distance between the chloride of one unit and the sodium of the next is at 4.153(5) (34) (a) Coffindaffer, T. W.; Rothwell, I. P.; Huffman, J. C. Inorg. Chem. 1983, 22, 2906. (b) Huffman, J. C.; Moloy, K. G.; Marsella, J. A.; Caulton, K. G. J. Am. Chem. Soc. 1980, 3009. (c) Evans, W. J.; Grate, J. W.; Bloom, I.; Hunter, W. E.; Atwood, J. L. J. Am. Chem. Soc. 1985, 107, 405. (d) Evans, W. J.; Hanusa, T. P.; Levan, K. R. Inorg. Chim. Acta 1985, 110, 191. (e) Chisholm, M. H.; Rothwell, I. P. ComprehensiVe Coordination Chemistry; Wilkinson, G., Ed.; Pergamon Press: Oxford, England, 1987; Vol. 2, p 351. (35) Evans, W. J.; Olofson, J. M.; Ziller, J. W. Inorg. Chem. 1989, 28, 4308. (36) Hitchcock, P. B.; Lappert, M. F.; Smith, R. G. Inorg. Chim. Acta 1987, 139, 183. (37) Schumann, H.; Winterfeld, J.; Ko¨hn, R. D.; Esser, L.; Sun, J.; Dietrich, A. Chem. Ber. 1993, 126, 907.
Figure 2. ORTEP drawing (40% probability) of {ClLu[OC6H2(CH2NMe2)2-2,6-Me-4]3Na} (3a) with the adopted numbering scheme.
Figure 3. PLUTON drawing of {ClLu[OC6H2(CH2NMe2)2-2,6Me-4]3Na} (3a) showing the view along the pseudo-3-fold axis (Cl in front).
Å smaller than the 4.765(3) Å found in the crystal packing of 3a, but still much larger than the sum of the covalent radii (2.53 Å). In contrast to the crystal packing of 3a, where both possible enantiomers are present in the measured crystal, only one of the four possible stereoisomers of 4 is present in the measured crystal. The relatively large space around these cylinders is filled with strongly disordered crystal solvent, which could not be modeled in the crystal structure determination. Structures in Solution. The solid-state structures are retained in solution, as appears from 1H and 13C NMR data. At room temperature the 1H NMR spectrum of 3a in C6D6 shows two broad signals for the NMe2 protons and four broad resonances for the benzylic protons. In addition, the 13C NMR in C6D6 shows two separate resonances for both the benzylic and NMe2 carbon atoms and single resonances for all aromatic carbon atoms. These data indicate that all phenolate ligands are equivalent in solution, with different binding modes for the
Binding in Yttrium and Lutetium Complexes
Figure 4. ORTEP drawing (30% probability) of {ClY[µ-OC6H4(CH2NMe2)-2]3Y[OC6H4(CH2NMe2)-2]3Na} (4) with the adopted numbering scheme.
Inorganic Chemistry, Vol. 35, No. 5, 1996 1191
Figure 6. Y-O bond length (Å) vs Y-O-C bond angles for complex 4. In this graph “1st shell” refers to the phenolate ligands bridging the two Y-atoms and “2nd shell” to the phenolate ligands bridging Y and Na in the molecular structure of 4. Table 6. Y-O Bond Lengths and Y-O-C Bond Angles in Yttrium Phenolates complex [Y(OC6H3Me2-2,6)3(THF)]2 (7) Y(OC6H3tBu2-2,6)3 (8) [(C8H8)Y(OC6H5)(THF)]2 (9)
(C5Me5)Y(OC6H3tBu2-2,6)2 (10) Y2NaCl[OC6H4(CH2NMe2)-2]6 (4)
Figure 5. PLUTON drawing of {ClY[µ-OC6H4(CH2NMe2)-2]3Y[OC6H4 (CH2NMe2)-2]3Na} (4) showing the view along the pseudo-3-fold axis (Cl in front).
two amino substituents. Room temperature NMR data for 3b are similar, although the signals for the benzylic protons are too broad to be observed. Interestingly, the resonance for the ipso-carbons in 3b is a doublet due to coupling with 89Y (100% abundance I ) 1/2), with 2JYC ) 2.2 Hz. To our knowledge, this is the first time an 89Y coupling has been observed with a phenolate ipso-carbon. At -40 °C in a toluene-d8 solution of 3b, the 1H NMR spectrum shows three singlet signals for the NMe2 protons: two integrating for 9 protons each at 1.43 and 1.63 ppm, and one integrating for 18 protons at 2.53 ppm. The resonances for the benzylic protons appear as two AX patterns with all four doublets integrating for three protons each. This shows that at this temperature the two amino substituents on each phenolate ligand experience different chemical environments (no rotation of the ligand around the C-O bond), while the association/ dissociation process of one of the two metal to nitrogen dative bonds is blocked on the NMR time scale. On account of the (38) Schaverien, C. J.; Frijns, J. H. G.; Heeres, H. J.; van den Hende, J. R.; Teuben, J. H.; Spek, A. L. J. Chem. Soc., Chem. Commun. 1991, 642.
Y-O (Å)
Y-O-C (deg)
2.075(6) 2.046(6) 2.00(1) 2.00(2) 2.00(1) 2.360(5) 2.294(4) 2.250(5) 2.259(4) 2.096(4) 2.059(3) 2.100(6) 2.096(7) 2.111(6) 2.255(6) 2.236(7) 2.256(6) 2.360(6) 2.391(6) 2.411(6)
162.6(5) 168.7(6) 175(1) 173(1) 171(1) 117.95 121.09 135.74 130.63 128.6(3) 154.0(9) 155.3(6) 154.9(5) 161.1(6) 139.0(5) 135.1(5) 138.9(6) 120.1(5) 118.9(5) 122.9(5)
ref 35 36 37
38 this work
stronger Lewis acidic character of the yttrium ion as compared to the sodium ion, the activation energy for Y-N dissociation can be expected to be higher than that for Na-N dissociation and the Y-N association/dissociation process will be the first to become slow on the NMR time scale. As a result, the NMe2 resonances at 1.43 and 1.63 ppm can be assigned to the amino substituents coordinated to yttrium. Consequently the Na-N dissociation/association process at this temperature is still fast on the NMR time scale, resulting in homotopic resonances. When the temperature is raised, line broadening and coalescence of the various resonances occurs. At room temperature, the resonances of the benzylic protons are so broad that they are observed with difficulty, while the presence of two broad NMe2 signals show that, although both the Y-N and Na-N association/dissociation processes have become fast on the NMR time scale, rotation of the ligand around the C-O bonds is still slow. At higher temperatures (343 K), the latter signals also coalesce, which can only be explained by rotation of the O-bonded phenolate ligands around the C-O bonds. These observations indicate that both 3a and 3b have similar structures with asymmetric Na-N and Y/Lu-N bonding of the bis(oamino)phenolate ligands.
1192 Inorganic Chemistry, Vol. 35, No. 5, 1996
Hogerheide et al.
Figure 7. Y-O bond lengths vs Y-O-C bond angles for yttrium phenolates. For references and complex numbering see Table 6. 1H and 13C NMR characterization of 4 indicates the presence of two different coordination geometries for the phenolate ligand and temperature dependent resonances. The 1H NMR spectrum at room temperature in CDCl3 shows two different AX patterns for the benzylic protons, while the NMe2 protons give rise to two separate signals (1.99 and 1.94 ppm) for one coordination geometry and to a single broad signal (1.62 ppm) for the other. Furthermore, the 13C NMR spectrum shows two separate signals for the ipso-carbon (164.24 and 160.01 ppm), as well as two separate resonances for the benzylic carbon atom and three for the NMe2 carbons. The presence of two separate resonances for the NMe2 hydrogen and carbon atoms for one of the two coordination geometries and a single resonance for the other shows that the association/dissociation process for the nitrogen to metal dative bond is slow on the NMR time scale for the former and fast for the latter. Using the same argument as mentioned above for 3b, the fast association/dissociation process can be assigned to the Na-N dative bonds. In addition, the NMR data show that exchange between the two coordination geometries does not take place on the NMR time scale. Also here, the resonances for the ipso-carbons both appear as doublets due to coupling with 89Y: the signal at 164.24 ppm shows a coupling of 4.0 Hz and the signal at 160.01 a coupling of 0.6 Hz. In addition to this, the 1H NMR spectrum shows a doublet for one aromatic proton that is shifted considerably upfield (5.80 ppm). Cooling a CDCl3 solution of 4 to 238 K slows the association/ dissociation process of the nitrogen dative bonds (further) down, causing also the broad singlet at 1.62 ppm in the 1H NMR spectrum to split up into two separate signals (1.58 and 1.78 ppm). All other resonances remain unchanged. Raising the temperature to 330 K in CDCl3 only leads to coalescence of the set of signals for the NMe2 group of one coordination geometry at 1.58 and 1.78 ppm. The two AX patterns for the benzylic protons are still present in the 1H NMR at 330 K, as well as the two separate signals for the NMe2 group of the other coordination geometry. This shows the rigid nature of the structure of 4. 89Y NMR. 89Y NMR spectra of 3b in C D at room 6 6 temperature show a single, broad resonance at 160.9 ppm relative to 3 M YCl3 in D2O. Raising the temperature to 325 K led to considerable sharpening of the signal. As a result of the negative NOE effect of 89Y, a considerable (negative) 89Y signal enhancement was observed for 4 on using the decoupler. 89Y spectra (H-decoupled) of 4 show two sharp
Figure 8. 89Y NMR spectrum of 4 in CDCl3 (1.5 M; H-decoupled; 40 transients): coupling structure obtained by increasing the number of data points from 16K to 132K followed by a Gaussian Fourier procedure.
resonances at 132.4 and 202.4 ppm, both appearing as doublets due to coupling with each other, with 2JYY ) 0.4 Hz (see Figure 8). This indicates that the molecular structure of 4 in solution also comprises two inequivalent yttrium atoms, while the presence of the 89Y89Y spin-spin coupling confirms that the number of connecting bonds is small, which correlates with the bridging phenolate ligands observed in the solid state structure. When the decoupler is not used, the signal at 202.4 ppm becomes broader and some extra, poorly resolved fine structure becomes visible; i.e., this signal is coupled to an indeterminate number of protons; the signal at 132.4 ppm remains relatively sharp. The assignment to the individual yttrium atoms of the two resonances observed by 89Y NMR for 4 remains, however, a problem. The additional coupling structure, observed on the 89Y signal at 202.4 ppm when the decoupler was not used, can be a result of (i) coupling of the NMe2 protons of the ligands in the first shell with Y(1) or (ii) coupling of the aromatic orthoprotons of the ligands in both shells with Y(2). An attempt to obtain further experimental data by a 2D Y-H correlation NMR experiment was unsuccessful. In addition, the 89Y chemical shift of 160.9 ppm found for 3b falls in between the two signals found for 4 (202.4 and 132.4 ppm) and does not provide additional information with respect to the assignment of the two 89Y signals of 4. As stated earlier, based on the solid state structure, in principle four stereoisomers of 4 are possible, while the NMR spectra (1H, 13C and 89Y) only show one set of signals. These four stereoisomers can be divided into two enantiomeric pairs: (i) one pair where the two shells of screw-type chirality are of opposite sign (MP/PM pair) and (ii) one pair where they are of equal sign (MM/PP pair). 1H and 13C NMR, both at room temperature and below room temperature, show a single set of signals for 4, indicating that only one of the two enantiomeric pairs is present in solution. Connected to this is the presence of a doublet for one aromatic ortho-proton in the 1H NMR spectrum of 4, which is shifted considerably upfield at 5.80 ppm, and a second one that is shifted slightly upfield at 6.51 ppm. In the solid state structure of either MP or PM, the aromatic ortho-
Binding in Yttrium and Lutetium Complexes Scheme 3. Cooperativity in Anion-Cation Bonding Leading to the Formation of 3a and 3b
proton of a ligand in the second shell is, as a result of the opposite signs of screw-type chirality, positioned in the shielding cone of the aromatic ring of a ligand in the first shell and vice versa. The average distance to the aromatic ring is 3.045(11) Å in the former case, while it is much longer at an average of 3.36(9) Å in the latter. This increased shielding of the orthoprotons would not be present in MM or PP, leading to the conclusion that also in solution only the MP/PM pair is present. This is to be expected, since steric repulsion between the aromatic rings in the separate shells is likely to be more pronounced in the MM/PP pair than in the MP/PM pair and the latter pair is therefore preferred. The fact that the 1H NMR spectra of the mono(o-amino)phenolate complex 4 hardly show fluxional behavior of the complex in solution (only for the amino substituents coordinated to sodium is the coalescence temperature below 330 K), is in contrast to the fluxional behavior of the bis(o-amino) complexes 3a and 3b (all coalescence temperatures are at 343 K or below). This may be explained by the staggered arrangement of the two shells of phenolate ligands in 4. In combination with the opposite signs of screw-type chirality this forms a rigid arrangement where rotation of any one ligand can occur only with simultaneous rotation, in the same direction, of all ligands (transition from PM to MP or vice versa). In addition, it may even be necessary for all nitrogen dative bonds to be dissociated for this transition between the two enantiomers to take place. As may be expected, this process is of high energy and therefore slow on the NMR time scale, as evidenced by the presence of the AX patterns for the benzylic protons even at 330 K. Discussion The bis(o-amino) complexes 3 and 4 are “ate” complexes with structural features that have not been previously observed. The process of formation of 3 and 4 can be described in terms of cooperative anion-cation bonding. In detail, the structure of 3a can be thought of as starting from a lutetium tris(phenolate), Lu[OC6H2(CH2NMe2)2-2,6-Me-4]3, which is sixcoordinate on account of the rigidity of the ligand systems. Coordination of chloride anion completes the coordination sphere around lutetium, leading to preorganization of the three remaining pendant amino-substituents (see Scheme 3) and formation of an organized N3O3 pocket. Due to the negative charge on the oxygen centers this pocket is able to positively bind the sodium cation. This cooperativity in anion-cation bonding can be seen as a result of the “excess” coordinating capability present in the bis(o-amino) substituted phenolate ligand. A somewhat similar self-assembling process has very recently been reported for the nickel(II) complex of 3-methoxysalicylaldimine (L2), (L2)2Ni, in which the trans-NiN2O2 chromophore in the monometallic complex changes its configuration to cis upon the addition of lithium, sodium or potassium salts. This change in the donor atom arrangement of the two ligands around
Inorganic Chemistry, Vol. 35, No. 5, 1996 1193 Scheme 4. Self-Assembly of Complex 4 through Positive Cooperativity in Anion-Cation Bonding
the nickel center results in the formation of an outer O4 pocket that is able to bind an alkali metal anion, reminescent of the preorganization of the N3O3 pocket in the complexes 3 and complex 4.39 When the mono(o-amino) substituted phenolate 1 is used instead of the bis(o-amino) substituted 2, the three pendant amino substituents, necessary to form the six-coordinate pocket for the sodium ion, are absent. However, from the solid state structure (see Figure 4), it can be seen that preorganization of the three phenolate ligands by coordination of chloride anion to a neutral, coordinatively unsaturated tris(phenolate) moiety Y[OC6H4(CH2NMe2)-2]3 (see Scheme 4), leads to a coordination geometry around Y(1) in 4 that is strikingly similar to the coordination geometry around Lu in 3a. Coordination of a second tris(phenolate) Y[OC6H4(CH2NMe2)-2]3 to the preorganized arrangement of phenolate oxygen atoms of the {ClY[OC6H4(CH2NMe2)-2]3}- moiety precludes the coordination of the amino-substituents of this second shell of phenolate ligands to the second yttrium atom (see coordination geometry around Y(2) in 4). Then, as a result of the preorganized arrangement of the three phenolate ligands in the {ClY[OC6H4(CH2NMe2)2]3}- moiety, the three phenolate ligands of the second shell are preorganized to form a N3O3 pocket. As a result of the negative charge of the resulting bimetallic complex, this N3O3 pocket is able to positively bind the sodium cation, resulting in a coordination geometry around sodium in 4 that closely resembles that in 3a. This view that the second yttrium atom (Y(2) in the molecular structure of 4, see Figure 4) coordinates to the preorganized arrangement of the three phenolate ligands around Y(1) explains the asymmetric nature of the phenolate bridges and thus the very acute Y(2)-O-C bond angles and long Y(2)-O bond lengths connected with the ligands in the first shell. In addition, it allows for the sense of screw-type chirality of the second shell of ligands to be determined by the sense of screw-type chirality of the first shell of ligands, leading to the exclusive formation of the PM/MP enantiomeric pair as observed by NMR (Vide supra). This shows that 4 is the result of the self-assembly of two different molecules, where the stereochemical information in one building block determines the overall stereochemistry of the resulting polymetallic structure. The striking structural similarities between the coordination geometries around Lu in 3a and Y(1) in 4, as well as around Na in both complexes, indicate that these geometries are very stable and we propose that the positive cooperativity in anion-cation bonding can be seen as the driving force for the self-assembly of complex 4. Furthermore, 4 can be seen as comprising the capping ends of an organometallic polymeric (39) Costes, J.-P.; Dahan, F.; Laurent, J.-P. Inorg. Chem. 1994, 33, 2738.
1194 Inorganic Chemistry, Vol. 35, No. 5, 1996
Figure 9. Schematical representation of an organometallic polymer that might be build up from the capping ends that together form complex 4.
material: {YCl[OC6H4(CH2NMe2)-2]3}- (starter) and {Y[OC6H4(CH2NMe2)-2]3Na}+ (stopper) for polymeric materials of general formula {YCl[OC6H4(CH2NMe2)-2]3}-[Y(OAr)3]n{Y[OC6 H4(CH2NMe2)-2]3Na}+ (see Figure 9). Design of these complexes involves the insertion of one or more shells of an yttrium tris(alkoxide) or tris(phenolate) complex Y(OR)3 (“spacers”) in between the starter and stopper; see Figure 9. In this respect, the use of phenolate complexes is especially interesting, as the screw-type chirality of both starter and stopper will induce screw-type chirality in the spacers, most probably resulting in rigid, rodlike coordination polymers. In principle it may even be possible to insert complexes of metals other than yttrium. Strategies to achieve this goal are currently being studied. Preliminary results of an experiment where complex 4 was mixed, in THF solution, with 1 equiv of Y(OC6H3Me2-2,6)3(THF)3 (7)35 indicate that 1 equiv of NaCl is liberated with the formation of an as yet unidentified (polymetallic) yttrium complex. So far we have not been able to grow crystals suitable for an X-ray structure determination. With respect to the preparation of preceramic mixed-metal complexes, the cooperativity in the bonding of anion and cation, resulting in the complexes 3 and 4, opens the possibility to incorporate cations other than Na+, either by exchange of the cation in the complexes after their preparation or by starting from the neutral metal tris(phenolates) and reacting these with
Hogerheide et al. the desired metal salt. Following the former strategy, attempts to substitute the chloride in both 3 and 4 with phenolate (OC6H5), alkoxide (OiPr, OTf), or alkyl (CH2SiMe3, CH3) monoanionic ligands either led to isolation of starting products (in the case of OC6H5) or to an undefined reaction mixture (all other attempts). These experiments, however, indicated that the use of lithium reagents to substitute the chloride leads to partial exchange of Na+ by Li+. In this respect it is interesting to note that the EI-MS spectrum of 3b shows the highest mass peak at 776 m/z, which corresponds to Na[M(OC6H4(CH2NMe2)-2)3]+, suggesting that, apart from a relative volatility of the complex, loss of Cl-anion from the molecular ion does lead to a stable cation. In conclusion, 3a, 3b, and 4 are unique complexes showing the versatility in coordination geometry of the applied monoor bis(o-CH2NMe2)-substituted phenolate ligands. The complexes open new perspectives for both the preparation of preceramic (hetero)polymetallic complexes for high temperature superconductor research and the design of self-assembling organometallic materials. In order to test the postulated cooperativity in anion-cation bonding, we are currently developing methods for the preparation of the salt-free Ln(OAr)3 complexes. Such complexes may also be useful for the selective complexation and activation of Lewis bases, since the site on the metal center, which in both 3 and 4 is occupied by a chloride anion, can in principle be tuned by binding different types of cations in the N3O3 cavity at the other side of the molecule. Acknowledgment. This work was financially supported (M.P.H.) by the Innovation Oriented Research Program on Catalysis (IOP-Katalyse) and supported in part (A.L.S. and W.J.J.S.) by the Netherlands Foundation for Chemical Research (SON) with financial aid from the Netherlands Organization for Scientific Research (NWO). Supporting Information Available: Tables giving further details on the structure determinations, including crystallographic data, atomic coordinates, bond lengths and angles, and thermal parameters for 3a and 4 (12 pages). Ordering information is given on any current masthead page. IC950639H
